depends on how many moles of reactants
4.96x1024
Stoichiometry relates moles of reactant to moles of product, so if you have the amount of reactant in the equation, you can calculate the amount of product produced.
1) Find moles of reactants 2) From moles of reactants calculate how many moles of products you'll get 3) Whichever gives you the most product is in excess
CO2 + 4H2 --> CH4 + 2H2O0.500 moles CO2 (1 mole CH4/1 mole CO2) = 0.500 moles CH40.500 moles CO2 (2 moles H2O/1 mole CO2) = 1.00 moles H2O-------------------------------------------------------------------------------------add= 1.50 moles total product====================
The coefficients give the ratio of moles reactant to moles product.
The maximum amount of product that can be formed is found by first writing out the balanced equation for the reaction. Calculate the number of moles of starting material you have (moles = mass/molar mass) Use the equation to figure out how many moles of product this will produce. Convert this to grams by multiplying by the mole mass (of the new substance this time.)
0,83moles glucose are burned.
8,54 mL toluene is equivalent to 0,08 moles.
Stoichiometry relates moles of reactant to moles of product, so if you have the amount of reactant in the equation, you can calculate the amount of product produced.
1) Find moles of reactants 2) From moles of reactants calculate how many moles of products you'll get 3) Whichever gives you the most product is in excess
CO2 + 4H2 --> CH4 + 2H2O0.500 moles CO2 (1 mole CH4/1 mole CO2) = 0.500 moles CH40.500 moles CO2 (2 moles H2O/1 mole CO2) = 1.00 moles H2O-------------------------------------------------------------------------------------add= 1.50 moles total product====================
The coefficients give the ratio of moles reactant to moles product.
3
Since the product, K2SO4 has twice as many potassium atoms as the reactant, KNO3, we may conclude that it takes two moles of reactant to produce one mole of product. The sulfate and nitrate ions will not be the limiting factor.
The maximum amount of product that can be formed is found by first writing out the balanced equation for the reaction. Calculate the number of moles of starting material you have (moles = mass/molar mass) Use the equation to figure out how many moles of product this will produce. Convert this to grams by multiplying by the mole mass (of the new substance this time.)
Assuming the reaction is S + O2 --> SO2, this equation is balanced as written, with everything in a 1:1 molar ratio. So, 67.1 moles of product would require 67.1 moles of O2 reactant.
To convert grams into moles the equation to be used is grams of product divided by the atomic weight of the product. So the equation would be 251.8 g/105.9886 g/mol= 2.3757272 mols
Moles of one substance compared to moles of the second substance. Ex. moles of reactant A compared to moles pf product F